The rate of a reaction quadruples when the temperature changes from 300 to 310K. What is the activation energy of this reaction?
(Assume activation energy and preexponential factor are independent of temperature ; In 2= 0.693; R= 8.314 J $m o l^{- 1} K^{- 1}$ )

Open in App

Solution

$log (\frac{k_{2}}{k_{1}}) = \frac{E_{A}}{2.303 R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$
$\Rightarrow log (4) = \frac{E_{A}}{2.303 \times 8.314} \times [\frac{1}{300} - \frac{1}{310}]$
$\Rightarrow 2 \times 0.693 = \frac{E_{A}}{2.303} \times \frac{0.0001075}{8.314}$
$\Rightarrow E_{A} = \frac{26.53793}{0.0001075} = 2.46 \times 10^{5} J m o l^{- 1}$

Suggest Corrections

Similar questions

Q. The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is :
(Assume activation energy and pre-exponential factor are independent of temperature;

l n 2

=0.693; R = 8.314 J

m o l^{- 1} K^{- 1}

)

Q. The rate of a reaction doubles when its temperature changes from

300 K

310 K

. Activation energy of such a reaction will be:

(R = 8.314 J K^{- 1} {m o l}^{- 1} a n d log 2 = 0.301)

Q. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

(R = 8.314 J K^{- 1} m o l^{- 1}

and

l o g_{10} 2 = 0.301)

Q. The rate of a reaction becomes four times when the temperature changes from

293 K

313 K

. Calculate the energy of activation

(E_{2})

of the reaction assuming that it does not change with temperature.

[R = 8.314 J / K m o l^{- 1}, log 4 = 0.6021]

The rate of a reaction doubles when its temperature changes form 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314 J K^{- 1} m o l^{- 1} a n d l o g 2 = 0.301)$

Join BYJU'S Learning Program

The rate of a reaction quadruples when the temperature changes from 300 to 310K. What is the activation energy of this reaction?(Assume activation energy and preexponential factor are independent of temperature ; In 2= 0.693; R= 8.314 Jmol−1K−1)

log(k2k1)=EA2.303R[1T1−1T2]⇒log(4)=EA2.303×8.314×[1300−1310]⇒2×0.693=EA2.303×0.00010758.314⇒EA=26.537930.0001075=2.46×105Jmol−1

The rate of a reaction quadruples when the temperature changes from 300 to 310K. What is the activation energy of this reaction?
(Assume activation energy and preexponential factor are independent of temperature ; In 2= 0.693; R= 8.314 J $m o l^{- 1} K^{- 1}$ )